Consider the reaction C12 H22O1 (s) +1202 (g)+12C02 (g)+ 11H20(1) in which 10.0 g of sucrose, C12 H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/ C. The temperature increase inside the calorimeter was found to be 22.0 °C. Calculate the change in internal energy, AE, for this reaction per mole of sucrose. Express the change in internal energy in kilojoules per mole to three significant figures. • View Available Hint(s) kJ/mol AE = Submit Previous Answers

Water gas is produced from the reaction of steam with coal: C(s)+H2O(g)H2(g)+CO(g) Assuming that coal is pure graphite, calculate H for this reaction.

Consider the reaction between methane and oxygen producing carbon dioxide and water. Suppose that the reaction is carried out in a furnace used to heat a house. If q=890kJ and w=+5kJ, what is E? H at 25C?

What is the heat gained/released at constant pressure equal1o (qp = ?)? What is the heat gained/released at constant volume equal to (qv = ?)? Explain why H is obtained directly from a coffee-cup calorimeter, whereas E is obtained directly from a bomb calorimeter.

9.61 Silane, SiH4, burns according to the reaction, SiH4+2O2SiO2+2H2O , with H=1429 kJ. How much energy is released if 15.7 g of silane is burned?

9.47 If 14.8 kJ of heat is given off when 1.6 g of HCl condenses from vapor to liquid, what is Hcond for this substance?

Syngas can be burned directly or converted to methanol. Calculate H for the reaction CO(g)+2H2(g)CH3OH(l)

9.63 Reactions of hydrocarhons are often studied in the petroleum industry. One example is 2C3H8(g)C6H6(l)+5H2(g) , with H = 698 kJ. If 35 L of propane at 25C and 0.97 atm is to be reacted, how much heat must he supplied?

When a 0.740-g sample of trinitrotoluene (TNT), C7H5N2O6, is burned in a bomb calorimeter, the temperature increases from 23.4 C to 26.9 C. The heat capacity of the calorimeter is 534 J/C, and it contains 675 mL of water. How much heat was produced by the combustion of the TNT sample?

A gaseous hydrocarbon reacts completely with oxygen gas to form carbon dioxide and water vapour. Given the following data, determine Hf for the hydrocarbon: Hreaction=2044.5KJ/molhydrocarbonHf(CO2)=393.5KJ/molHf(H2O)=242KJ/mol Density of CO2 and H2O product mixture at 1.00 atm, 200.c = 0.751g/L. The density of the hydrocarbon is less than the density of Kr at the same conditions.